Pre CH13 HW for Silberberg
Followings are what you will find at the end of the chapter in your textbook.
For LEARNING OBJECTIVES: Highlight the main idea for EACH objective. Ready carefully so you
don’t highlight everything.
For MASTER THESE SKILLS: Highlight the main idea for each skill. Ready carefully so you don’t
highlight everything.
For KEY TERMS: Make sure you can define it and/or give an example of it. Pick TWO terms of your
choice and actually write the definition or an example.
For KEY EQUATIONS AND RELATIONSHIP: Next to EACH, define each term. Be very specific.
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CHAPTER REVIEW GUIDE
Learning Objectives Relevant section (§) and/or sample problem (SP) numbers appear in parentheses.
Understand These Concepts
1.
2.
3.
4.
5.
6.
7.
8.
The quantitative meaning of solubility (§13.1)
The major types of intermolecular forces in solution and their relative strengths (§13.1)
How the like-dissolves-like rule depends on intermolecular forces (§13.1)
Why gases have relatively low solubilities in water (§13.1)
General characteristics of solutions formed by various combinations of gases, liquids, and solids (§13.1)
How intermolecular forces stabilize the structures of proteins, the cell membrane, and DNA (§13.2)
The enthalpy components of a solution cycle and their effect on ΔHsoln (§13.3)
The dependence of ΔHhydr on ionic charge density and the factors that determine whether ionic solution
processes are exothermic or endothermic (§13.3)
9. The meaning of entropy and how the balance between the change in enthalpy and the change in entropy
governs the solution process (§13.3)
10. The distinctions among saturated, unsaturated, and supersaturated solutions, and the equilibrium nature
of a saturated solution (§13.4)
11. The relation between temperature and the solubility of solids (§13.4)
12. Why the solubility of gases in water decreases with a rise in temperature (§13.4)
13. The effect of gas pressure on solubility and its quantitative expression as Henry's law (§13.4)
14. The meaning of molarity, molality, mole fraction, and parts by mass or by volume of a solution, and
how to convert among them (§13.5)
15. The distinction between electrolytes and nonelectrolytes in solution (§13.6)
16. The four colligative properties and their dependence on number of dissolved particles (§13.6)
17. Ideal solutions and the importance of Raoult's law (§13.6)
18. How the phase diagram of a solution differs from that of the pure solvent (§13.6)
19. Why the vapor over a solution of volatile nonelectrolyte is richer in the more volatile component (§13.6)
20. Why electrolyte solutions are not ideal and the meanings of the van't Hoff factor and ionic atmosphere
(§13.6)
21. How particle size distinguishes suspensions, colloids, and solutions (§13.7)
22. How colloidal behavior is demonstrated by the Tyndall effect and Brownian motion (§13.7)
Master These Skills
1. Predicting relative solubilities from intermolecular forces (SP 13.1)
2. Calculating the heat of solution for an ionic compound (SP 13.2)
3. Using Henry's law to calculate the solubility of a gas (SP 13.3)
4. Expressing concentration in terms of molality, parts by mass, parts by volume, and mole fraction (SPs
13.4, 13.5)
5. Interconverting among the various terms for expressing concentration (SP 13.6)
6. Using Raoult's law to calculate the vapor pressure lowering of a solution (SP 13.7)
7. Determining boiling point elevation and freezing point depression of a solution (SP 13.8)
8. Using a colligative property to calculate the molar mass of a solute (SP 13.9)
9. Calculating the composition of vapor over a solution of volatile nonelectrolyte (§13.6)
10. Calculating the van't Hoff factor (i) from the magnitude of a colligative property (§13.6)
11. Using a solution depiction to determine colligative properties (SP 13.10)
Key Terms Page numbers appear in parentheses.
Section 13.1
solute (518)
solvent (518)
miscible (518)
solubility (S) (518)
like-dissolves-like rule (518)
hydration shell (518)
ion–induced dipole force (518)
dipole–induced dipole force (518)
alloy (522)
Section 13.2
protein (523)
amino acid (523)
soap (525)
lipid bilayer (526)
nucleic acid (527)
mononucleotide (527)
double helix (527)
Section 13.3
heat of solution (ΔHsoln) (528)
solvation (529)
hydration (529)
heat of hydration (ΔHhydr) (529)
charge density (529)
entropy (S) (531)
Section 13.4
saturated solution (533)
unsaturated solution (533)
supersaturated solution (533)
Henry's law (535)
Section 13.5
molality (m) (537)
mass percent [% (w/w)] (538)
volume percent [% (v/v)] (538)
mole fraction (X) (538)
Section 13.6
colligative property (541)
electrolyte (541)
nonelectrolyte (541)
vapor pressure lowering (ΔP) (542)
Raoult's law (542)
ideal solution (542)
boiling point elevation (ΔTb) (543)
freezing point depression (ΔTf) (545)
semipermeable membrane (546)
osmosis (546)
osmotic pressure (Π) (546)
fractional distillation (548)
ionic atmosphere (549)
Section 13.7
suspension (552)
colloid (552)
Tyndall effect (553)
hard water (554)
water softening (554)
ion exchange (554)
reverse osmosis (555)
desalination (555)
wastewater (555)
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Key Equations and Relationships Page numbers appear in parentheses.

13.1 Dividing the general heat of solution into component enthalpies (528):

13.2 Dividing the heat of solution of an ionic compound in water into component enthalpies (530):

13.3 Relating gas solubility to its partial pressure (Henry's law) (535):

13.4 Defining concentration in terms of molarity (537):

13.5 Defining concentration in terms of molality (537):

13.6 Defining concentration in terms of mass percent (538):

13.7 Defining concentration in terms of volume percent (538):

13.8 Defining concentration in terms of mole fraction (538): Mole fraction (X)

13.9 Expressing the relationship between the vapor pressure of solvent above a solution and its mole
fraction in the solution (Raoult's law) (542):

13.10 Calculating the vapor pressure lowering due to solute (542):

13.11 Calculating the boiling point elevation of a solution (544):

13.12 Calculating the freezing point depression of a solution (545):

13.13 Calculating the osmotic pressure of a solution (546):
Answer the following questions. Show your work.
(a) What is the relationship between (direct, inverse or not related?) vapor pressure and strength of
intermolecular forces?
(b) What is the relationship between (direct, inverse or not related?) polarity of the molecule and strength of
intermolecular forces?
(c) What is the relationship between (direct, inverse or not related?) vapor pressure and boiling point?
(d) What is the relationship between (direct, inverse or not related?) boiling point and molar mass?
(e) What is the relationship between (direct, inverse or not related?) energy and stability?
(f) What is the relationship between (direct, inverse or not related?) stability and reactivity?
(g) Explain in your own words what Colligative property is.
(h) Explain in your own words what “like dissolve like” mean